(Chem 200) 01- Matter, Measurment, And Problem Solving

Front 1

Atoms and molecules determine how matter __________.

Back 1

behaves

Front 2

Carbon monoxide (CO)

Back 2

a colorless gas emitted in the exhaust of vehicles

Front 3

Atoms:

Back 3

the submicroscopic particles that constitute the fundamental building blocks of ordinary matter

Front 4

molecule:

Back 4

two or more atoms joined in a specific geometric arrangement.

Front 5

Hemoglobin:

Back 5

the oxygen carrying protein in blood.

Front 6

How does carbon monoxide affect us?

Back 6

it happens to be just the right size and shape, and happens to have just the right chemical properties to fit neatly into cavities w/in hemoglobin normally reserved for oxygen.
- CO diminishes the oxygen carrying capacity of blood.
- over 0.04% can kill you
- small amounts will cause the heart and lungs to work harder resulting in headaches, dizziness, weakness, confusion.

Front 7

Difference between CO and CO2:

Back 7

Front 8

Chemistry:

Back 8

The science that seeks to understand the behavior of matter by studying the behavior of atoms and molecules.

Front 9

Empirical knowledge:

Back 9

based on an observation and experiment

Front 10

Qualitative:

Back 10

noting/ describing how a process happens

Front 11

Quantitative:

Back 11

measuring or quantifying something about the process

Front 12

Hypothesis:

Back 12

a tentative interpretation or explanation of the obervations

Front 13

Experiments:

Back 13

test hypotheses, highly controlled procedures designed to generate observations.

Front 14

Scientific law:

Back 14

a brief statement that summarizes past observations and predicts future ones.
- describes how nature behaves

- generalization about what nature does.

Front 15

Law of conservation of mass:

Back 15

"in a chemical reaction, matter is neither created nor destroyed."

Front 16

Scientific Theory:

Back 16

a model for the way nature is and tries to explain not merely what nature does but why.

Front 17

Atomic Theory:

Back 17

- proposed by John Dalton (1766-1844)

- matter is composed of small, indestructible particles (atoms). Since these particles are merely rearranged in chemical changes (& not created/destroyed), total amount of mass remains the same.

Front 18

well-established _______ are as close to the truth as we get in science.

Back 18

theories

Front 19

The Scientific Method:

Back 19

Front 20

which of the following best explains the difference between a law and a theory?

a) a law is truth whereas a theory is mere speculation.

b) a law summarizes a series of related observations, while a theory gives the underlying reasons for them.

c) a theory describes what nature does; a law describes why nature does it.

Back 20

B) a law summarizes a series of related observations, while a theory gives the underlying reasons for them.

Front 21

Matter:

Back 21

anything that occupies space and has mass.

ex:
book, desk, human, air

Front 22

Substance:

Back 22

a specific instance of matter

ex:
air, water, sand

Front 23

What are the 3 states of matter?

Back 23

Front 24

Solid matter:

Back 24

- atoms or molecules packed close to each other in fixed locations.

- although the atoms and molecules in a solid vibrate, they do not move around or past each other.

- has a fixed vol. and rigid shape

Front 25

solids may be _______ or _________.

Back 25

Crystalline, amorphous

Front 26

Crystalline:

Back 26

in solid matter, its atoms or molecules are arranged in patterns with long-range, repeating order.

Front 27

Amorphous:

Back 27

in solid matter, its atoms or molecules do not have any long-range order

Front 28

Liquid matter:

Back 28

atoms or molecules pack about as closely as they do in a solid matter, but they are free to move relative to each other.

- fixed vol., but not a fixed shape

- assume shape of their container

Front 29

gaseous matter:

Back 29

atoms or molecules have a lot of space between them and are free to move relative to one another making gases compressible.

- always assume the shape and vol. of their container.

Front 30

How to classify matter according to its composition:

Back 30

Front 31

Composition:

Back 31

the kinds and amounts of substances that composes matter

Front 32

Pure Substance:

Back 32

a substance composed of a single type of atom or molecule.

ex: distilled (pure) water

Front 33

Pure substances can be divided into what two types?

Back 33

elements, compounds

Front 34

Elements:

Back 34

a substance that cannot be chemically broken down into simpler substances.

ex: Helium

Front 35

Compounds:

Back 35

a substance composed of two or more elements in fixed, definite proportions.

ex: water

Front 36

Mixture:

Back 36

a substance composed of two or more different types of atoms or molecules that can be combined in continuously variable proportions.

Front 37

mixtures can be divided into what two types?

Back 37

heterogeneous mixtures, homogeneous mixtures

Front 38

Heterogeneous mixtures:

Back 38

one in which the composition varies from one region to another.

ex: wet sand

Front 39

homogeneous mixture:

Back 39

one with the same composition throughout.

ex: sweet tea

Front 40

Physical Change:

Back 40

changes that alter only state or appearance but not composition.

ex:
water that boils changes state from liquid to gas but composition of molecules are not changed.

Front 41

chemical Change:

Back 41

Changes that alter the composition of matter.

- atoms rearrange

ex: rusting iron.

Front 42

Chemical Change:

Back 42

Changes that alter the composition of matter.

- atoms rearrange

Front 43

physical property:

Back 43

a property that a substance displays without changing its composition

Front 44

Chemical property:

Back 44

a property that a substance displays only by changing its composition via chemical change.

Front 45

what are some physical properties:

Back 45

- odor
- taste
- color
- appearance
- melting pt.
- boiling pt.
- density

Front 46

Chemical properties include:

Back 46

- corrosiveness
- flammability
- acidity
- toxcitiy

Front 47

example of physical change and chemical change:

Back 47

Front 48

Back 48

(a) best represents the water after vaporization. Vaporization is a physical change, so the molecules must remain the same before and after the change.

Front 49

Energy:

Back 49

the capacity to do work

Front 50

Work:

Back 50

the action of a force through a distance

Front 51

total energy:

Back 51

kinetic energy + potential energy

Front 52

Kinetic energy:

Back 52

energy associated with its motion

Front 53

Potential energy:

Back 53

energy associated with its position/ composition

Front 54

thermal energy:

Back 54

energy associated with the temperature of a object.

- actually a type of kinetic energy because it arises from the motion of the individual atoms/ molecules that make up an object.

Front 55

example of energy conversion:

Back 55

Front 56

Law of conservation of energy:

Back 56

"energy is neither created nor destroyed"

the total quantity of energy does not change-- remains constant.

Front 57

"systems with high potential energy have a tendency to change in a way that lowers their potential energy"

Back 57

summary:
- energy is always conserved in a physical or chemical change; it is neither created nor destroyed.

- systems with high potential energy tend to change in a direction of lower potential energy, releasing energy into the surroundings.

Front 58

units:

Back 58

standard quantities used to specify measurement.

Front 59

International system of units (SI):

Back 59

used by scientists based on metric system.

Front 60

SI base Units:

Back 60

Front 61

1kg = how many lbs?

Back 61

2.205lbs

Front 62

temperature scales:

Back 62

Front 63

converting from fahrenheit to celsius:

Back 63

Front 64

SI prefix Multipliers:

Back 64

Front 65

Derived unit:

Back 65

combination of other units

Front 66

volume:

Back 66

a measure of space

Front 67

some common units and their equivalents:

Back 67

Front 68

Density:

Back 68

- a characteristic physical property of materials and differs from one substance to another

- an intensive property

Front 69

Intensive property:

Back 69

one that is independent of the amount of the substance

Front 70

extensive property:

Back 70

one that depends on the amount of the substance.

Front 71

Back 71

(c) the sample expands. However, because the mass remains constant, its density decreases.

Front 72

Significant figures rules:

Back 72

Front 73

Exact numbers:

Back 73

have no uncertainty, and thus do not limit the number of significant figures in any calculation.

Front 74

rules for calculating sig. figs:

Back 74

Front 75

accuracy:

Back 75

how close the measured value is to the actual value

Front 76

precision:

Back 76

how close a series of measurements are to one another or how reproducible they are.

Front 77

example of errors:

Back 77

- inconsistency is the result of random error (error that has equal probability of being too high or too low)

- inaccuracy is the result of systematic error (error that tends toward being either too high or too low)